Question

Aluminum reacts with chlorine gas to form aluminum chloride via the following reaction: 2Al(s)+3Cl2(g)→2AlCl3(s) What is the maximum mass of aluminum chloride that can be formed when reacting 32.0 g of aluminum with 37.0 g of chlorine? Express your answer to three significant figures and include the appropriate units.

Answer 1

Answer: The mass of aluminium chloride that can be formed are 46.3 g

Explanation:

To calculate the number of moles, we use the equation:

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$  ....(1)  

• For Aluminium:

Given mass of aluminium = 32 g  

Molar mass of aluminium = 26.98 g/mol

Putting values in above equation, we get:  

$\text{Moles of aluminium}=\frac{32g}{26.98g/mol}=1.186mol$

• For Chlorine:

Given mass of chlorine = 37 g  

Molar mass of chlorine = 71 g/mol

Putting values in above equation, we get:  

$\text{Moles of chlorine gas}=\frac{37g}{71g/mol}=0.521mol$

For the given chemical equation:

$2Al(s)+3Cl_2(g)\rightarrow 2AlCl_3(s)$

By Stoichiometry of the reaction:

3 moles of chlorine gas is reacting with 2 moles of aluminium.

So, 0.521 moles of chlorine gas will react with = $\frac{2}{3}\times 0.521=0.347moles$ of aluminium.

As, given amount of aluminium is more than the required amount. Thus, it is considered as an excess reagent.

So, chlorine gas is considered as a limiting reagent because it limits the formation of products.

By Stoichiometry of the reaction:

3 moles of chlorine gas is producing 2 moles of aluminium chloride

So,  0.521 moles of chlorine gas will react with = $\frac{2}{3}\times 0.521=0.347moles$ of aluminium chloride.

Now, calculating the mass of aluminium chloride by using equation 1, we get:

Moles of aluminium chloride = 0.347 moles

Molar mass of aluminium chloride = 133.34 g/mol

Putting all the values in equation 1, we get:

$0.347mol=\frac{\text{Mass of aluminium chloride}}{133.34g/mol}\\\\\text{Mass of aluminium chloride}=46.3g$

Hence, the mass of aluminium chloride that can be formed are 46.3 g

Answer 2

The quantity of the substance is given by the mass. The mass of aluminium chloride formed when reacting aluminium with chlorine will be 46.3 gm.

What is mass?

Mass is a quantitative factor that determines the amount of substance or matter present in the sample.

The chemical reaction can be shown as,

$\rm 2 Al + 3Cl_{2} \rightarrow 2AlCl_{3}$

Calculate the number of moles of Aluminium:

$\begin{aligned}\rm Moles & = \dfrac {\rm Mass }{\rm Molar\; mass}\\\\& = \dfrac{32}{26.98}\\\\& = 1.186\;\rm moles\end{aligned}$

Calculate the number of moles of Chlorine:

$\begin{aligned}\rm Moles & = \dfrac {\rm Mass }{\rm Molar\; mass}\\\\& = \dfrac{37}{71}\\\\& = 0.521 \;\rm moles\end{aligned}$

From the stoichiometry of the reaction above:

2 moles of aluminium reacts with 3 moles of chlorine

So, moles of aluminium will react with 0.521 moles chorine is,

$\dfrac{2}{3} \times 0.521 = 0.347 \;\rm moles$

From this, it can infer that chlorine gas is a limiting reagent and aluminium is an excess reagent.

From the stoichiometry of the reaction,

3 moles of chlorine =  2 moles of aluminium chloride

So, 0.521 moles chorine will give,

$\dfrac{2}{3} \times 0.521 = 0.347 \;\text{ moles of aluminium chloride.}$

Calculate the mass of the aluminium chloride as:

$\begin{aligned} \rm mass &= \rm moles \times molar\; mass\\\\&= 0.347 \times 133.34\\\\&= 46.3 \;\rm g\end{aligned}$

Therefore, the mass of the aluminium chloride is 46.3 gm.

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